Chemistry 0620/32 May/June 2025: question paper and mark scheme

Question

A list of substances is shown. aluminium bromine calcium carbon dioxide iron magnesium magnesium oxide neon oxygen potassium sulfur dioxide Answer the following questions about these substances. Each substance may be used once, more than once or not at all. State which substance is: (a) an element which forms an ion with a 2– charge …… [1] (b) an ionic compound …… [1] (c) used as a catalyst …… [1] (d) approximately 21% of clean, dry air …… [1] (e) a gas needed for photosynthesis …… [1] (f) the most reactive metal in the list …… [1] (g) a gas that is tested for using acidified aqueous potassium manganate(VII) …… [1] (h) a noble gas …… [1] (i) in Group VII. …… [1] [Total: 9]

Question

This question is about sea water and the substances found in sea water. (a) Table 2.1 shows the masses of some of the compounds formed when 500 cm3 of sea water is evaporated. Table 2.1 compound formula mass of compound / g sodium chloride NaCl 7.0 MgSO4 2.5 potassium bromide KBr 1.5 calcium carbonate CaCO3 1.0 Answer these questions using the information from Table 2.1. (i) State the chemical name of MgSO4. …… [1] (ii) The total mass of compounds formed from 500 cm3 of sea water is 12.0 g. Calculate the total mass of compounds formed from 750 cm3 of sea water. mass = …… g [1] (iii) State which compound in Table 2.1 reacts with an acid to produce carbon dioxide. …… [1] (b) Potassium bromide is found in sea water and contains bromide ions. Describe a test for bromide ions. test …… observations …… [2] (c) Calcium ions are in sea water. Complete Fig. 2.1 to show: • the electronic configuration of a calcium ion • the charge on the ion. Ca Fig. 2.1 [2] (d) Sodium chloride is a solid at room temperature. Describe the arrangement and motion of the particles in a solid. arrangement …… motion …… [2] (e) Sea water contains dissolved nitrate ions. State one source of nitrate ions. …… [1] [Total: 10]

Question

This question is about phosphorus and its compounds. (a) (i) Phosphorus is in Group V of the Periodic Table. Explain why phosphorus is placed in this group. …… [1] (ii) Two isotopes of phosphorus are shown in Fig. 3.1. 31 32 15P 15P Fig. 3.1 Complete Table 3.1 to show the number of protons, neutrons and electrons in one atom of these isotopes. Table 3.1 protons neutrons electrons 31 15P 32 15P [3] (iii) Phosphorus burns in oxygen to produce phosphorus(V) oxide. Complete the symbol equation for this reaction. ……P + ……O2 P4O10 [2] (iv) State whether phosphorus(V) oxide is an acidic oxide or a basic oxide. Give a reason for your answer. …… [1] (b) (i) Phosphorus is one element in NPK fertilisers. Draw a circle around one other element that is also in NPK fertilisers. krypton nickel platinum potassium [1] (ii) State why farmers use fertilisers on fields where crops are grown. …… [1] (c) A compound of phosphorus has the formula Ca3(PO4)2. Complete Table 3.2 to calculate the relative formula mass of Ca3(PO4)2. Table 3.2 number of relative atomic atom atoms mass oxygen 8 16 8 × 16 = 128 calcium 40 phosphorus 31 relative formula mass = …… [2] [Total: 11]

Question

This question is about organic chemistry. (a) (i) State the meaning of the term hydrocarbon. …… [1] (ii) Petroleum is a mixture of hydrocarbons. Outline how petroleum is separated into its useful components. Include in your answer: • the name of the separation technique • the property of the hydrocarbons which allows them to be separated • a description of how this technique separates the petroleum into its useful components. …… [4] (iii) Some of the products obtained from petroleum are shown. Draw a line from each product to its use. product use kerosene making roads bitumen fuel for cars gasoline jet fuel [2] (b) Ethanol is an organic molecule. (i) Draw the displayed formula of a molecule of ethanol. [2] (ii) Ethanol is manufactured by the reaction of steam with ethene. State two conditions for this process. 1 …… 2 …… [2] (c) Fig. 4.1 shows the displayed formula of tetramethylsilane. H H C H H H H C Si C H H H H C H H Fig. 4.1 (i) Deduce the molecular formula of tetramethylsilane. …… [1] (ii) Name the two elements in tetramethylsilane that are in the same group in the Periodic Table. …… and …… [1] [Total: 13]

Question

This question is about zinc salts. (a) Excess solid zinc oxide is added to dilute sulfuric acid to produce a salt. (i) Complete the word equation for this reaction. zinc oxide sulfuric acid …… + + …… [2] (ii) Name the method used to remove excess solid zinc oxide from the reaction mixture. …… [1] (iii) Describe how crystals of the pure salt are made from an aqueous solution of the salt formed. …… [2] (b) Fig. 5.1 shows the apparatus for the electrolysis of molten zinc chloride using inert electrodes. – power + supply heat Fig. 5.1 (i) Label Fig. 5.1 to show the: • cathode • electrolyte. [2] (ii) Name a suitable material for the inert electrodes. …… [1] (iii) Name the products formed at the positive and negative electrodes. positive electrode …… negative electrode …… [2] (c) Zinc chloride has ionic bonds. State the meaning of the term ionic bond. …… [2] [Total: 12]

Question

This question is about metals. (a) (i) A student investigates the reaction of four different metals, A, B, C and D, with dilute hydrochloric acid. All other conditions are the same in each test‑tube. The results of the experiment are shown in Fig. 6.1. bubbles A B C D Fig. 6.1 Put the metals, A, B, C and D, in order of their reactivity. most reactive …… least reactive …… [1] (ii) The student wants to decrease the rate of the reaction in the experiment. State two ways to decrease the rate of this reaction. 1 …… 2 …… [2] (b) In another experiment, a student adds potassium carbonate to dilute hydrochloric acid. State the colour seen in the flame test for potassium ions. …… [1] (c) Brass is a mixture of two metals. (i) State the name given to a mixture of metals such as brass. …… [1] (ii) Name the two metals in brass. …… and …… [2] (iii) Magnalium is a mixture of magnesium and aluminium. Suggest one property of magnalium that makes it more useful than pure magnesium metal. …… [1] [Total: 8]

Question

(a) Select two processes that show a chemical change. Tick (3) two boxes. boiling water burning methane dissolving salt mixing ink and water rusting of iron [2] (b) The reaction of hydrogen with nitrogen is a reversible reaction. Write the symbol that shows a reversible reaction. …… [1] (c) Table 7.1 shows the results of four experiments. Table 7.1 experiment initial temperature / °C final temperature / °C 1 18 23 2 19 17 3 18 14 4 19 29 (i) State which experiment shows the greatest temperature change. …… [1] (ii) State which experiment is the most endothermic. …… [1] (iii) In experiment 4, magnesium was added to dilute hydrochloric acid. Complete the symbol equation. Mg + ……HCl MgCl 2 + …… [2] (iv) Fig. 7.1 shows an incomplete reaction pathway diagram for an endothermic reaction. progress of reaction Fig. 7.1 Complete Fig. 7.1 by labelling: • the vertical axis • the reactants • the products. [2] [Total: 9]

Question

This question is about water and air. (a) Water needs to be treated to make it safe to drink. Draw a line from each stage in the treatment of domestic water to the reason why it is carried out. stage reason addition of carbon to kill microbes to remove tastes sedimentation and odours chlorination to remove solids [2] (b) Describe how to test whether a sample of water is pure using melting point. …… [2] (c) Air may contain sulfur dioxide and particulates. (i) State one harmful effect of each of these air pollutants. sulfur dioxide …… particulates …… [2] (ii) Describe how flue gas desulfurisation reduces emissions of sulfur dioxide gas. …… [2] [Total: 8] The Periodic Table of Elements Group I II III IV V VI VII VIII 1 2 H He hydrogen helium Key 1 4 3 4 atomic number 5 6 7 8 9 10 Li Be atomic symbol B C N O F Ne lithium beryllium name boron carbon nitrogen oxygen fluorine neon 7 9 relative atomic mass 11 12 14 16 19 20 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar sodium magnesium aluminium silicon phosphorus sulfur chlorine argon 23 24 27 28 31 32 35.5 40 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr potassium calcium scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine krypton 39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium tin antimony tellurium iodine xenon 20 85 88 89 91 93 96 – 101 103 106 108 112 115 119 122 128 127 131 55 56 57–71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 lanthanoids Cs Ba Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn caesium barium hafnium tantalum tungsten rhenium osmium iridium platinum gold mercury thallium lead bismuth polonium astatine radon 133 137 178 181 184 186 190 192 195 197 201 204 207 209 – – – 87 88 89–103 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 actinoids Fr Ra Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og francium radium rutherfordium dubnium seaborgium bohrium hassium meitnerium darmstadtium roentgenium copernicium nihonium flerovium moscovium livermorium tennessine oganesson – – – – – – – – – – – – – – – – – 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu lanthanum cerium praseodymium neodymium promethium samarium europium gadolinium terbium dysprosium holmium erbium thulium ytterbium lutetium 139 140 141 144 – 150 152 157 159 163 165 167 169 173 175 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr actinium thorium protactinium uranium neptunium plutonium americium curium berkelium californium einsteinium fermium mendelevium nobelium lawrencium – 232 231 238 – – – – – – – – – – – The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).